STUDY CHECK 9.1 Calculate the total mass of the reactants and the products for the following...
Use reaction stoichiometry to calculate amounts of reactants and products. The substances ammonia and oxygen gas react to form nitrogen monoxide and water. Unbalanced equation: NH; (g) + O2(g) — NO(g) + H20 (g) In one reaction, 66.9 g of H2O is produced. What amount (in mol) of O2 was consumed? What mass (in grams) of NO is produced? mol O2 consumed g NO produced
Calculate the total masses of the reactants for the following equation: 2Al(s)+3Cl2(g)→2AlCl3(g)
The combination of Mg and O2. Write the chemical equation (reactants, products, and states of matter) Mg(s) + O2(g) -> MgO2(s)?
Consider the following equilibrium systems. Which direction will the reactions shift (reactants or products) when cooled? 2CO(g) + O2(g) = 2CO2(8) H2(g) + 12(g) = 2HI(g) H2(g) + 12(s) = 2H1(2) 12(g) = 21(2) AH = -566 kJ AH = -2.70 kJ AH = +53.0 kJ AH = +36.2 kJ _ a. reactants, reactants, reactants, reactants b.reactants, reactants, products, products c. products, products, products, products d. products, products, reactants, reactants | 0 0 0 0
1.) Enter your answer in the provided box Calculate the mass % of O in barium periodate ? % O 2.) Be sure to answer all parts. Write a balanced equation for the following by inserting the correct coefficients. If the coefficient equals 1, add "1" in the provided box. ??? CaSiO3(s) + ???? HF(g) → ??? CaF2(s) + ??? SiF4(g) + ???H2O(l) 3.) Be sure to answer all parts. Potassium nitrate decomposes on heating, producing potassium oxide and gaseous...
How do we find the total mass of excess reactants? Cryolite, Na, AIF,(), an ore used in the production of aluminum, can be synthesized using aluminum oxide. Balance the equation for the synthesis of cryolite. equation: A1,0,($) +6 NaOH(1) + 12 HF(g) 2 Na, AIF+9H2O(g) If 13.4 kg of Al,0,(s), 51.4 kg of NaOH(I), and 51.4 kg of HF(g) react completely, how many kilograms of cryolite will be produced? mass of cryolite produced: 55 kg Na, AlF Which reactants will...
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g)...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (d) 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) KP = 16.5; initial pressures: SO3 = 1.00 atm, SO2 = 1.00 atm, O2 = 1.00 atm (e) 2NO(g) + Cl2 (g) ⇌ 2NOCl(g) Kc = 4.6 × 104 ; [NO] = 1.00 M, [Cl2] = 1.00...
6. (1 pt) Which represents an ENDOTHERMIC reaction? a. 10 kJ + reactants - products b. reactants-> products + 10 kJ C reactants - products d. reactants-products 7. (1 pt) Which represents a reaction that requires a catalyst? a. 10 kJ + reactants-> products b. reactants -> products + 10 kJ c. reactants products d. reactants-> products 8. (1 pt) Which represents reversible reaction? a. 10 kJ + reactants -> products b. reactants-> products + 10 kJ C. reactants products...
1. The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and use it to determine the direction in which each system will proceed to reach equilibrium. Write "R" if the reactions shifts to the right towards products or "L" if it shifts left towards reactants. A. {NO} = 1.00 M, {Cl2} = 1.00 M, {NOCl} = 0.00 M; K = 4.6 x 104 2NO(g)+Cl2(g)<->2NOCl(g) B. {SO3} = 2.00...