1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C,H,(NO,).) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. 2. Suppose 30.0 L of carbon dioxide gas are produced by this reaction, at a 15.0 °C and pressure of exactly 1 atm. Calculate the mass of temperature of nitroglycerin that must have reacted. Be sure your answer has the correct number of significant digits.

Calculate the red part given the data

Carla and her friends were tasked with determining the heat of reaction for the neutralization of the newly synthesized monoprotic acid HX and NaOH. The rubber ball calorimeter was initially calibrated using the reaction of 7.0 mL of 0.200 M HCl and 14.0 mL of 0.1000 M KOH. This measured a temperature rise from 15.7 °C to 27.9 °C. After that, the heat of reaction was calculated for a combination of 2.00 mL of 1.00 M NaOH and 5.0 mL of 1.00 M HX. This represented a temperature rise of 3.7 degrees Celsius. What is the calorimeter's heat capacity in J/°C? (Δ??????????????? =-50.85 kJ/mol)? For the reaction between NaOH and HX, create the chemical and net ionic equations that are equally balanced.

Assuming constant pressure, a gas has a final volume of 15 L. If the temperature increases from 330 K to 450 K, find the initial volume. Show all work in the space provided, and then write your final answer on the short line.