True or False? A mole of CH4 has the same mass as a mole of CCl4
Mass of one mole of CH4= 16 g
Mass of one mole of CCl4= 12+(4*35.5) = 154 g
So the correct option is false
A mole of a substance has the same mass in grams as one unit (atom or molecules) has in atomic mass units. True False
a) consider the following reaction CH4 +4Cl2 = CCl4+ 4HCl what mass of CCl4 is formed by the reaction of 4.80g of methane with an excess of chlorine? and why b) Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by the equation: 4NH3 + 5O2 = 4NO + 6H2O What mass of NO can be produced from 7.76 g of NH3? and why?
The reaction CH4 (8) + CCl4 (g) = 2 CH2Cl2 (B) has an enthalpy change AHI° - 18.8 kJ. You allow the equation to proceed to equilibrium at 25 °C, then raise the temperature to 50 °C. How will the equilibrium concentrations be affected by this temperature change? Concentrations of CH4 and CCl4 will increase. Concentration of CH2Cl2 will increase. Concentrations of CCl4 and CH2Cl2 will increase The concentrations will remain the same.
1 mole of NO2(e) has a greater entropy than 1 mole of N204(g). True or false False O True
True or False: A half mole of CO2 and a half mole of CS2 have the same number of molecules. and the complete combustion of butane, C4H10 produces CO2 and H2O.
Consider the following system at equilibrium at 350 K: 2CH2Cl2(g) CH4(g) + CCl4(g) When some CH4(g) is removed from the equilibrium system at constant temperature: The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CCl4 will: A. Increase. B. Decrease. C. Remain the same.
For the reaction CH4 + 4Cl2 CCl4 + 4HCl, how many grams of Cl2 are needed to make 55.2 g of CCl4?
1. Rank the following in order of increasing mass: 1.0 mole of methane (CH4), 0.50 mole of water (H2O), 0.20 mole of Fe, and 0.010 mole of U. 2. When heated, calcium carbonate (limestone) undergoes a decomposition reaction. Write a balanced equation for this reaction.
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g)----> CH4(g) + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.59×10-2 M CH2Cl2, 0.181 M CH4 and 0.181 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.134 mol of CCl4(g) is added to the flask? [CH2Cl2] = _____ M [CH4] = _____ M [CCl4] = _____ M
Consider the following chemical reaction: CH4 (g) + Cl2(g) + CCl4 (1) + CCl4 (I) + HCl (g) Identify the type of chemical reaction that this is classified as: oxidation-reduction (redox) O precipitation + acid-base precipitation + redox precipitation acid-base