When CO(g) reacts with H₂O(1) to form CO₂(g) and H₂(g), 0.669 kcal of energy are absorbed for each mole of CO(g) that reacts. Write a balanced equation for the reaction with an energy term in kcal as part of the equation. Use the SMALLEST INTEGER coefficients possible and put the energy term in an appropriate box. If a box is not needed, leave it blank. Submit Answer + + -> Retry Entire Group 8 more group attempts remaining + +

Answer the following questions about the chemical reaction shown below.O3 (g) + H2O (g) →  H2 (g) + 2 O2 (g) ΔH = 3.0 kcal/mol A flask contains the components of the reversible chemical reaction shown above, at equilibrium. Describe how the system will respond if each of the following stresses are applied. a) The flask is heated. ________________________________________________ b) The pressure in the flask is increased. ________________________________ c) Oxygen gas is selectively removed from the flask. _____________________

Can you answer it as if you where putting it in those boxes. Set the equation up

For the following reaction, 4.98 grams of silver nitrate are mixed with excess copper(II) chloride. The reaction yields 2.90 grams of silver chloride. silver nitrate (aq) + copper(II) chloride (s) - →silver chloride (s) + copper(II) nitrate (aq) What is the ideal yield of silver chloride? What is the percent yield for this reaction? % grams

Consider the following balanced reaction. How many moles of C3H7SH are needed to produce 0.214 moles of CO2? Assume excess O2. C3H7SH() + 6 02g) → 3 CO2(8) + SO2(g) + 4 H20 (g) Your Answer: Answer units

Calculate the % yield for problem number 9 if only 500.0 g of NBr3 are actually made from 525 g Br2  N2   +   3 Br2   →   2 NBr3   +   44.0 kJ                                  actual yield                  ______________  g NBr3 % yield = ------------------------ 100 =-------------------------- 100 =  _____________  %                  theoretical yield             ________________  g NBr3

Answer the questions that provide the information.

For the following balanced equation:  CH4 + 4 Cl2 ==> CCl4 + 4 HCl Determine the number of moles of HCl that  can be made from 6.80 moles of CH4? Answer to 2 decimal places.

Question 49 In 1-2 sentences, explain what the Arrhenius equation tells us. Use the diagram to help describe what you mean. 100 °C - room temperature (300 °K) k, = Ae¯FalRT (373 °K) 4 kJ/mol (1 kcal/mol) 40 kJ/mol (10 kcal/mol) 80 kJ/mol (19 kcal/mol) → energy (E) Edit Format Table 12pt v Paragraph v BI Ų Av ev T? v * s fraction of molecules having energy E

For the reaction shown, find the limiting reactant for each of the following initial amounts of reactants. 2 Na(s) + Br₂(g) → 2 NaBr(s) 2 mol Na, 2 mol Br₂ Express your answer as a chemical formula. Part B A chemical reaction does not occur for this question. Submit Request Answer 1.8 mol Na, 1.4 mol Brą Express your answer as a chemical formula. Submit ΑΣΦ Part C A chemical reaction does not occur for this question. Request Answer ΑΣΦ Submit [MD] 2.5 mol Na. 1 mol Brą Express your answer as a chemical formula. Part D ΑΣΦ A chemical reaction does not occur for this question. Request Answer 12.6 mol Na. 6.9 mol Brą Express your answer as a chemical formula. ΑΣΦ ? ? A chemical reaction does not occur for this question.