A sample of gas contains 0.1600 mol of CH4(g) and 0.1600 mol of H2O(g) and occupies...

A sample of gas contains 0.1600 mol of CH4(g) and 0.1600 mol of H2O(g) and occupies a volume of 12.1 L. The following reaction takes place: CH4(g) + H2O(g)-----3H2(g) + CO(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. ____(?)Liters

Expert Solution

queen_honey_blossom answered 2 years ago

A sample of gas contains 0.1000 mol of HCl(g) and 5.000×10-2 mol of Br2(g) and occupies...

A sample of gas contains 0.1000 mol of HCl(g) and 5.000×10-2 mol of Br2(g) and occupies a volume of 4.79 L. The following reaction takes place: 2HCl(g) + Br2(g)2HBr(g) + Cl2(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. A sample of gas contains 0.1800 mol of HCl(g) and 9.000×10-2 mol of Br2(g) and occupies a volume of 9.74 L. The following reaction takes place: 2HCl(g) + Br2(g)2HBr(g)...

A mixture of 0.05263 mol of H2O, 0.01327 mol of CH4, 0.07198 mol of CO, and...

A mixture of 0.05263 mol of H2O, 0.01327 mol of CH4, 0.07198 mol of CO, and 0.06917 mol of H2 is placed in a 1.0-L steel pressure vessel at 1303 K. The following equilibrium is established: 1 H2O(g) + 1 CH4(g) 1 CO(g) + 3 H2(g) At equilibrium 0.009871 mol of CH4 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of H2O, CH4, CO, and H2. Peq(H2O) = . Peq(CH4) = . Peq(CO) = . Peq(H2)...

10. A mixture of 0.08729 mol of H2O, 0.1041 mol of CH4, 0.08069 mol of CO,...

10. A mixture of 0.08729 mol of H2O, 0.1041 mol of CH4, 0.08069 mol of CO, and 0.1098 mol of H2 is placed in a 1.0-L steel pressure vessel at 1034 K. The following equilibrium is established: 1 H2O(g) + 1 CH4(g) 1 CO(g) + 3 H2(g) At equilibrium 0.06283 mol of CO is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of H2O, CH4, CO, and H2. Peq(H2O) = ____ . Peq(CH4) = ____ . Peq(CO)...

For the equilibrium system CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g),...

For the equilibrium system CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g), ΔH = -206 kJ/mol, state whether the yield of CH4 will increase, decrease or remain the same for the following changes: Adding some H2 gas to the system Removing H2O from the system Increasing the volume of the system Decreasing the temperature on the system Adding a catalyst to the system

A 1.0 mol sample of helium gas and a 1.0 mol sample of ammonia gas are...

A 1.0 mol sample of helium gas and a 1.0 mol sample of ammonia gas are held at the same temperature. Assuming both behave as ideal gases, do they have the same total internal energy?

A 0.02862 g sample of gas occupies 10.0 mL at 290.5 K and 10 atm. Upon...

A 0.02862 g sample of gas occupies 10.0 mL at 290.5 K and 10 atm. Upon further analysis, the compound is found to be 38.734% C and 61.266% F. What is the molecular formula of the compound? Draw the Lewis structure of the compound. Is the compound polar? What is the geometry around each carbon atom?

A 0.02887 g sample of gas occupies 10.0 mL at 288.0 K and 1.10 atm. Upon...

A 0.02887 g sample of gas occupies 10.0 mL at 288.0 K and 1.10 atm. Upon further analysis, the compound is found to be 38.734% C and 61.266% F. What is the molecular formula of the compound? Identify the geometry around each carbon atom. Is this compound polar?

A 10.00 g sample of a hydrate of magnesium chloride (MgCl2•x H2O) contains 5.317 g of...

A 10.00 g sample of a hydrate of magnesium chloride (MgCl2•x H2O) contains 5.317 g of H2O. What is the value of x?

16.05 g of methane (CH4) gas is mixed with 101.12 g of oxygen (O2) gas. The...

16.05 g of methane (CH4) gas is mixed with 101.12 g of oxygen (O2) gas. The mixture is ignited. After a bright flash and a loud bang, some water droplets form on the inside of the reaction vessel. A) Write the balanced chemical reaction for the combustion of methane . B) How many moles of water can you make? C) How many moles of CO2 can you make? D) Will anything be left over? What? Yes, there will be oxygen...

Suppose that 0.330 mol of methane, CH4(g), is reacted with 0.480 mol of fluorine, F2(g), forming...

Suppose that 0.330 mol of methane, CH4(g), is reacted with 0.480 mol of fluorine, F2(g), forming CF4(g) and HF(g) as sole products. Assuming that the reaction occurs at constant pressure, how much heat is released? Using data sheet below: Substance ΔH∘f (kJ/mol) C(g) 718.4 CF4(g) − 679.9 CH4(g) − 74.8 H(g) 217.94 HF(g) − 268.61

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