Be sure to answer all parts. Given the reaction represented by the balanced equation CH4(g) + 3Br2(g) → 3HBr(g) + CHBr3(g)
Calculate the number of g of CHBr3 produced by mixing 110 g Br2 with excess CH4.
Be sure to answer all parts. Given the reaction represented by the balanced equation CH4(g) +...
Question 12 (of 23) - > 12. Be sure to answer all parts. Given the reaction represented by the balanced equation CH,6) +316) + 3HI(g) + CHT() Part 1: Calculate the number of g of CHI, produced by mixing 140 g 1, with excess CH- T2,4 CH Part 2 out of 2 If 49.0 g CHI, were actually produced, calculate the % yield. % yield MacBook Air
CHEMISTRY n #2 < Question 12 (of 23) Reg Be sure to answer all parts. Given the reaction represented by the balanced equation CH,®) + 31,8)- 3HI) + CHI (8) Would try an of this Part 1 out of 2 By d Calculate the number of g of CHI, produced by mixing 140 g 1, with excess CH- scratch points with I CHI Next part MacBook Air
6. Given the reaction represented by the balanced equation: Sn(s) + 2 HF (aq) - SnF2(s) + H2(8) a. Calculate the number of grams of SnF2 that can be produced theoretically by mixing 10.00 g of Sn with excess HF. b. If only 11.00 g of SnF, were produced, calculate the percent yield,
help! Be sure to answer all parts. Enter a net ionic equation for the following reaction (including states of matter): CaCl2(aq) + MnSO4(aq) → Write the net ionic equation (including physical states) for the reaction of NaBr(ag) with AgNO3(aq). Click in the answer box to activate the palette. Be sure to answer all parts. Calculate the number of g of o, that will react with 6.28 mol of CzHg. Enter your answer in scientific notation. The balanced equation is: C3Hg(8)...
Be sure to answer all parts. Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) + 2NH3(g) Calculate the mass of ammonia produced when 33.0 g of nitrogen react with 11.2 g of hydrogen. Which is the excess reactant and how much of it will be left over when the reaction is complete? o hydrogen nitrogen
5. Consider the following balanced equation and answer parts (a) through (g). Show calculations for each part. 3 Ag(s) + 4HNO3(aq) + 3 AgNO3(aq) + NO(g) + 2 H2O(1) a) Calculate the number of moles of AgNO3 produced by the reaction of 3.10 moles of Ag with excess ΗΝΟ: b) Calculate the number of moles of AgNO, produced by the reaction of 108.21 grams of Ag with excess HNO
Be sure to answer all parts. Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3(s) - MgO(s) + CO2(g) AH - 117.3 kJ (a) Is heat absorbed or released in the reaction? absorbed released (b) What is A n for the reverse reaction? -1173 EJ (c) What is AH when 5.20 mol of CO, reacts with excess Mgo? (a) What is AH when 32.5 g of CO, reacts with exces: Mgo?
Be sure to answer all parts. Consider the following balanced thermochemical equation for a reaction sometimes used for H2S production: =Sg(s) + H2(g) → H2S() AH rxn = -20.2 kJ his an exothermic or endothermic reaction? endothermic exothermic (b) What is AH rxn for the reverse reaction? KJ (c) What is AH when 3.10 mol of Sg reacts? kJ
Be sure to answer all parts. The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 2.20 moles of HBr in a 18.1−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium. [H2] =___ M Br2] = ___M [HBr] = ____M
Be sure to answer all parts. Write a balanced equation for the following by inserting the correct coefficients (if a coefficient = enter "1" in the provided box): (CN)2(g) + H20(1) ► NH3(g) + H2C204(aq)