According to the balanced reaction below, calculate the moles of NHs that form when 4.2 mol of N:H. completely reacts N:H«(1) → 4 NH3(g) + N:(g)

Each step in the following process has a yield of 60.0%. CCl₂ + 4HCI → CCL₂F₂ + 2HCl The CCI, formed in the first step is used as a reactant in the second step. If 5.00 mol CH₂ reacts, what is the total amount of HCI produced? Assume that Cl₂ and HF are present in excess. CH4 + 4Cl₂ CCl₂ + 2 HF moles HCl: 12.48 Incorrect mol

In the following equations to determine which reactant is the limiting reactant and which reactant is in excess to NaOH + H2SO4 equals Na2SO 4 + H2O 10.0g.     10.0g

How many grams of N2 are needed to completely (stoichiometrically) react with 222 g of Br2 ? N2 + 3 Br2 2 NB13 + 44.0 kJ The molar mass of Br2 is g and the molar mass of N2 is mol Br2 (2.22 x 102 g Br2)(- mol Br2 g Br2 mol N2 mol Br2 (-- -) = mol N2 mol Br2 g N2 mol N2 (-- -) = |v g N2 mol N2 а. 1 b. 2 С. 3 d. 4 е. 5 f. 253.719 g. 3.38 х 100 h. 3.26 x 103 i. 44.0 j. 1.33 x 102 k. 9.77 x 103 I. 4.44 x 102 m. 6.66 x 10² n. 500.0 o. 556 р. 90.0 q. 3.2852 r. 159.81 s. 28.013 t. 1.750 u. 0.8750 v. 13.0 w. 0.46306 х. 1.3892 у. 24.5 z. 38.5 аа. 2.190 bb. evolved Cc. absorbed dd. exothermic ee. endothermic

How many moles of water are produced when 6.33 moles of CH4 react? CH4 (g) + 2O2 (g) --> CO2 (g) + 2H2O (g) (balanced)

In a particular experiment 0.0039 moles of AgNO3 is added to 0.001875 NH4Cl and 0.156g of AgCl are recovered. What is the percent yield? AgNO3(aq) + NH4Cl(aq) --> AgCl(s) + NH4NO3(aq)

If 45.0 g of O2 are mixed with 6.70 g of H2 and the mixture is ignited, what massof water is produced?

Consider the reaction below. Calculate how much H2O (l), in grams, can be produced if 2.5 moles of H2 is allowed excess O2? 2 H2 (g) + O2 (g) à 2 H2O (l)

Suppose a 250. mL flask is filled with 1.0 mol of CO, 0.70 mol of H₂O and 2.0 mol of H₂. This reaction becomes possible: CO(g) + H₂O(g) CO₂(g) + H₂(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of CO₂. You can leave out the M symbol for molarity. initial change equilibrium 2 со 0 H₂O CO₂ X H₂ 0 X 5

Suppose that 10.0g of each reactant are added to a reaction chamber causing the following reaction: SO2 + NaOH = Na2SO3 + H2O what is the yield of Na2SO3 in grams? Which reactant is in excess? Which reactant is limiting? Which reactant has some left over after the reaction finishes? How much reactant is left over