Given the reaction below: R (s) + L (l)  -->  2 J (g) How many liters of J (g) can be collected at a temperature of 298.4 K and a pressure of 0.978 atm if 2.292 grams of R (s) are allowed to completely react? The molar mass of R is 64.5 g/mol.

The total pressure for this reaction is 1.4 torr: CH4(g) reacts with O2(g) to make CO2(g) and H2O(g) Calculate the partial pressure of H2O(g)

Consider the following reaction where Ko = 1.20×10-2 at 500 K. PCI5(g) PCI3(g) + Cl2(g) A reaction mixture was found to contain 0.114 moles of PCI5(g), 2.37×10-2 moles of PCI3(g), and 4.01x10-2 moles of Cl2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

For the following equation, how would you increase the amount of product? CO(g) + H2(g) → C(s) + H₂O(g) AH = -131.5 kJ/mole Remove carbon, decrease PH₂O, increase temperature, increase PCO, increase PH₂, decrease total pressure. Remove carbon, decrease PH₂O, decrease temperature, increase PCO, increase PH₂, decrease total pressure. Remove carbon, decrease PH₂O, decrease temperature, increase PCO, increase PH₂, increase total pressure. CDecrease PH₂O, decrease temperature, increase PCO, increase PH₂, increase total pressure. CDecrease PH₂O, decrease temperature, increase PCO, increase PH2, decrease total pressure. CDecrease PH₂O, increase temperature, increase PCO, increase PH₂, increase total pressure. Decrease PH₂O, increase temperature, increase PCO, increase PH₂, decrease total pressure. Remove carbon, decrease PH₂O, increase temperature, increase PCO, increase PH₂, increase total pressure.