When 20.5 g CH4 (MM = 16.04 g/mol) and excess Cl2 undergo a reaction that has a 90.5% yield, what mass of chloromethane (CH3Cl, MM = 50.48 g/mol) forms?
CH4(g) + Cl2(g) --> CH3Cl(g) + HCl(g)
When 20.5 g CH4 (MM = 16.04 g/mol) and excess Cl2 undergo a reaction that has...
Chloromethane forms by the reaction CH4(g) + Cl2(g) ⇌ CH3Cl(g) + HCl(g) at 1500K, Kp = 1.6 x 104 . In the reaction mixture, PCH4 = 0.13 atm, PCl2 = 0.035 atm, PCH3Cl = 0.24 atm, and PHCl = 0.47 atm. Is CH3Cl or CH4 forming?
When 27.4 g of methane and 40.4 g of chlorine gas undergo a reaction that has a 78.5% yield, what mass of chloromethane (CH3CI) forms? Hydrogen chloride also forms. g CH2C1
When excess Cl2 at constant pressure reacts with 0.300 mol of CH4(g) 295 kJ of energy evolves. Calculate the value of ΔH for this reaction, as written. CH4(g) + Cl2(g) → CHCl3(l) + H2(g) ΔH = ? a) -1970 kJ b) -1770 kJ c) +1970 kJ d) -983 kJ e) +1770 kJ
A-The following reaction has a Kp=1.6 x 104 at 1500 K. CH4(g) + Cl2(g) CH3Cl(g) + HCl(g) a. In a reaction mixture, PCH4 = 0.13atm , PCl2 = 0.035atm , PCH3Cl = 0.24atm , and PHCl = 0.47atm . Is the system at equilibrium? If not how does the reaction proceed to reach equilibrium? At equilibrium, the following stresses are applied. How is the equilibrium affected? Explain. i. HCl is removed. ii. CH3Cl is added iii. The volume is reduced...
When 88.9 g of calcium and 59.8 g of nitrogen gas undergo a reaction that has a 88.8% yield, what mass of calcium nitride forms?
When 77.6 g of calcium and 33.0 g of nitrogen gas undergo a reaction that has a 84.8% yield, what mass of calcium nitride forms? g calcium nitride
Molar Volume 11. What is the volume of 0.60 g of methane (CH4 MM = 16.04 g/mol) at STP? STP? many grams of methane (CHE MM = 16.04 g/mol) are there in 7.00 7,00 L of the past Ideal Gas Law 0.278 8 of a mystery gas hydrocarbon occupies a volume of 0.400 L at 5 pressure of 886 mmHg. What is the molar mass of this gas, and what is L at 55.0°C and a what is its identity...
Enter your answer in the provided box. When 27.4 g of methane and 40.4 g of chlorine gas undergo a reaction that has a 78.5% yield , what mass of chloromethane (CH3CI) forms? Hydrogen chloride also forms. g CH,CI Book
3.8 points An initial state before reaction of CH4 and Cl2 is shown in the figure. Based on the balanced equation and the figure, what is the excess reactant? CH (8) + 4 C12(g) → CCI.(g) + 4 HCl(g) HCI CCl4 CH4 Cl2
7. (a) Consider the chlorination of methane, given below: 1 CH4(g) + 4 Cl2(g) 1 CCl4(g) + 4 HCl(g) If CH4(g) is decreasing at the rate of 0.490 mol/s, what are the rates of change of Cl2(g), CCl4(g), and HCl(g)? Cl2(g)/t = ____ mol/s CCl4(g)/t = _____mol/s HCl(g)/t = _____mol/s (b) The decomposition reaction given below: 2 IF5(g) 1 I2(g) + 5 F2(g) is carried out in a closed reaction vessel. If the partial pressure of IF5(g) is decreasing at...