• 2) A 1.604-g sample of methane (CH4) gas and 6.400 g of oxygen gas are sealed in a 2.50-L vessel at 411 oC and?

    A 1.604-g sample of methane (CH4) gas and 6.400 g of oxygen gas are sealed in a 2.50-L vessel at 411 oC and are allowed to reach equilibrium. Methane can react with oxygen to form gaseous carbon dioxide and water vapor or methane can react with oxygen to form gaseous carbon monoxide and water vapor. At equilibrium the pressure of oxygen is 0.326... show more
    A 1.604-g sample of methane (CH4) gas and 6.400 g of oxygen gas are sealed in a 2.50-L vessel at 411 oC and are allowed to reach equilibrium. Methane can react with oxygen to form gaseous carbon dioxide and water vapor or methane can react with oxygen to form gaseous carbon monoxide and water vapor. At equilibrium the pressure of oxygen is 0.326 atm, and the pressure of water vapor is 4.45 atm. Calculate pressures of carbon monoxide and carbon dioxide at equilibrium.
    2 answers · Chemistry · 7 years ago
  • HELP!! Calculate the solubility of silver chloride in a solution that is 0.180 M in NH3.?

    Calculate the solubility of silver chloride in a solution that is 0.180 in NH3 . can you explain the steps please? thanks!!
    Calculate the solubility of silver chloride in a solution that is 0.180 in NH3 . can you explain the steps please? thanks!!
    1 answer · Chemistry · 8 years ago
  • How long does it take a radio signal from the Voyager spacecraft to reach Earth if the distance between Voyage?

    may you please explain its for my chemistry homework please & thank you
    may you please explain its for my chemistry homework please & thank you
    1 answer · Chemistry · 8 years ago
  • Chemistry question about percent composition, please help!?

    A gas mixture contains 0.3 moles each of carbon dioxide, acetylene (C2H2), and methane (CH4). It also contains 0.1 moles of an unknown gas. The total mass of the gas mixture is 28.628 g. Subsequently it is determined that the elemental composition of the mixture of gases by weight is: 54.16% carbon, 33.85% oxygen and 6.99% hydrogen. What is the... show more
    A gas mixture contains 0.3 moles each of carbon dioxide, acetylene (C2H2), and methane (CH4). It also contains 0.1 moles of an unknown gas. The total mass of the gas mixture is 28.628 g. Subsequently it is determined that the elemental composition of the mixture of gases by weight is: 54.16% carbon, 33.85% oxygen and 6.99% hydrogen. What is the chemical formula of the fourth, unknown gas?
    2 answers · Chemistry · 8 years ago
  • PLEASE NEED HELP, Determining unknown values of boron hydride?

    A 10-L flask is evacuated and weighed. It is found to have a mass of 456.3450 g. Into this flask is placed stoichiometric amounts of a boron hydride (BxHy) and oxygen. The total mass of the flask is then determined and found to be 465.0013 g. The total pressure in the flask is found to be 0.85736 atm at a temperature of 100.0C. Under these... show more
    A 10-L flask is evacuated and weighed. It is found to have a mass of 456.3450 g. Into this flask is placed stoichiometric amounts of a boron hydride (BxHy) and oxygen. The total mass of the flask is then determined and found to be 465.0013 g. The total pressure in the flask is found to be 0.85736 atm at a temperature of 100.0C. Under these conditions, boron hydrides, which are gases, react with oxygen to produce solid boron oxide and gaseous water. The total pressure in the flask after the reaction is found to be 0.64302 atm at a temperature of 100.0C. Determine the values of X and Y for the boron hydride and then write a balanced equation for the reaction. R = 0.08205821 LxatmKxemol. i really do not understand what this question is asking i would please appreciate the help thank you
    1 answer · Chemistry · 9 years ago
  • Determine the value of Kc for the reaction 2N2O (g) + 3O2 (g)-->2N2O4 (g)?

    Given the equilibrium constant values N2 (g) + 1/2 O2 (g) -->N2) (g) Kc=2.7 x 10E-18 N2O4 (g) --> 2NO2 (g) Kc = 4.6 x 10E-3 1/2 N2 (g) + O2 (g) -->NO2 (g) Kc = 4.1 x 10E-9.
    Given the equilibrium constant values N2 (g) + 1/2 O2 (g) -->N2) (g) Kc=2.7 x 10E-18 N2O4 (g) --> 2NO2 (g) Kc = 4.6 x 10E-3 1/2 N2 (g) + O2 (g) -->NO2 (g) Kc = 4.1 x 10E-9.
    2 answers · Chemistry · 9 years ago
  • Balancing RedOx Reactions in Acidic or Basic Aqueous Solution?

    Compose the balanced reaction equation for the following reaction occuring in basic aqueous medium. Reduce all coefficients to the lowest possible integers. Include H2O(l) and OH−(aq) appropriately to complete the equation. Fe(CN)64−(aq) + Ce4+(aq) → Ce(OH)3(s) + Fe(OH)3(s) + CO32−(aq) + NO3−(aq) YOU'RE HELP IS GREATLY APPRECIATED !... show more
    Compose the balanced reaction equation for the following reaction occuring in basic aqueous medium. Reduce all coefficients to the lowest possible integers. Include H2O(l) and OH−(aq) appropriately to complete the equation. Fe(CN)64−(aq) + Ce4+(aq) → Ce(OH)3(s) + Fe(OH)3(s) + CO32−(aq) + NO3−(aq) YOU'RE HELP IS GREATLY APPRECIATED ! THANKS IN ADVANCE
    1 answer · Chemistry · 9 years ago
  • Physics problem help plzzzzzz?

    100gm of lead at 100 c 200 gm of iron at 120 c and 50 gm of zinc at 210 c were dropped inside a copper calorimeter of mass 600 gm containing 246 gm of water at an initial temp 20 c deduce the final temp of the system given that the specific heat of lead is 0.03 of iron 0.11 and of each of zinc and copper is 0.09
    100gm of lead at 100 c 200 gm of iron at 120 c and 50 gm of zinc at 210 c were dropped inside a copper calorimeter of mass 600 gm containing 246 gm of water at an initial temp 20 c deduce the final temp of the system given that the specific heat of lead is 0.03 of iron 0.11 and of each of zinc and copper is 0.09
    1 answer · Chemistry · 10 years ago
  • Please help with this chemistry problem?

    A sample of hydrocarbon is combusted in O2(g) to produce 28.38 g of CO2(g), 5.811 g of H2O(g) and 404 kJ of heat...What is the mass of the hydrocarbon that was combusted? What is the value of ΔH°f per empirical-formula unit of the hydrocarbon? I found the mass of the hydrocarbon to be 8.394 g and the empirical formula to be CH...however, I'm not... show more
    A sample of hydrocarbon is combusted in O2(g) to produce 28.38 g of CO2(g), 5.811 g of H2O(g) and 404 kJ of heat...What is the mass of the hydrocarbon that was combusted? What is the value of ΔH°f per empirical-formula unit of the hydrocarbon? I found the mass of the hydrocarbon to be 8.394 g and the empirical formula to be CH...however, I'm not sure how to calculate the enthalpy of formation per empirical formula unit...
    2 answers · Chemistry · 1 decade ago
  • Calculate the molar solubility of Cr(OH)3 in 0.32 M NaOH.

    Kf for Cr(OH)4- is 8x10^(29) Steve O is correct that different textbooks have different values of Ksp - I've got Ksp = 6.7x10^(-31) but he's given me enough to go on to work the problem. and he's also correct about the answer being given with one significant figure. i worked this problem as shown below w/ a Ksp of 6.7x10^-31 and took... show more
    Kf for Cr(OH)4- is 8x10^(29) Steve O is correct that different textbooks have different values of Ksp - I've got Ksp = 6.7x10^(-31) but he's given me enough to go on to work the problem. and he's also correct about the answer being given with one significant figure. i worked this problem as shown below w/ a Ksp of 6.7x10^-31 and took that Ksp times the given Kf value to obtain 0.536 Ksp x Kf = 0.536 and when I multiply that by 0.32 I get 0.17152 So, I tried entering 0.2 as an answer but it was incorrect. I then tried 0.17 - also incorrect. I just wonder if anyone sees anything wrong or knows why these answers are incorrect
    Chemistry · 1 decade ago
  • Chem help please ::: Calculate the pH of a buffer that is 0.125 M in NaHCO3 and 0.105 in Na2CO3.?

    please show me the steps and how you got to the answer thank you so much!!!! also.... 2) A beaker with 155 ml of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.1M . A student adds 8.90 ml of a 0.340 M HCl solution to the beaker. How much will the pH change? The... show more
    please show me the steps and how you got to the answer thank you so much!!!! also.... 2) A beaker with 155 ml of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.1M . A student adds 8.90 ml of a 0.340 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.76. 10 points to best answer!!!! thanks even if you only help with one that is a great help!!!
    2 answers · Chemistry · 1 decade ago
  • A constant volume vessel contains 12.5g of a gas at 21 Celsius degree.?

    If the pressur4e of the gas is to remain constant as the temperature is raised to 210 celsius degre, how many grams of gas must be released?
    If the pressur4e of the gas is to remain constant as the temperature is raised to 210 celsius degre, how many grams of gas must be released?
    1 answer · Chemistry · 1 decade ago
  • Balancing equations?

    I need help writing the equations and balancing them, best answer to anyone who does them all and gets them right!! Thanks in advance!!!!!! - NaOH + CuSo4 -----> - BaCl2 + NaSO4 -----> -HCl + NaOH ------> - Zn(NO3)2 + CuSO4 -----> - Pb(NO3)2 + KI ----->
    I need help writing the equations and balancing them, best answer to anyone who does them all and gets them right!! Thanks in advance!!!!!! - NaOH + CuSo4 -----> - BaCl2 + NaSO4 -----> -HCl + NaOH ------> - Zn(NO3)2 + CuSO4 -----> - Pb(NO3)2 + KI ----->
    4 answers · Chemistry · 1 decade ago