grams of gasoline to raise CO by 1000 ppm at STP??

Assume that an incorrectly adjusted lawn mower is operated in a garage such that the combustion reaction in the engine is: C8H18 + (17/2)O2 -> 8CO + 9H2O If the dimensions of the garage are 3.0 by 5.0 by 5.0 meters, how many grams of gasoline must be burned to raise the level of CO in the air to 1000 ppm by volume at STP? Hint: Calculate volume of garage, mol carbon monoxide, get mass octane from chemical equation I could do it with formaldehyde but I'm lost on the gasoline...I tried and tried, ughh

Nernst applic: atm pressure? given pH, Fe3+=Fe2+?

What is the calculated value of the partial pressure(atm) of O2 in acid mine water of pH 1.700, in which [Fe3+] = [Fe2+]? It seemed simple enough...I looked at other examples but couldn't find one on lead having equal concentrations.

mass of carbon needed to increase average CO2 by 170 ppm

Taking the mass of the atmosphere to be 4.3E15 metric tons, what mass of carbon must be burned in order to increase the average carbon dioxide level in the atmosphere by 170ppm by volume (in metric tons)? I only have one try left on the computer!!! I downloaded a couple of study guide examples but the were wrong. Please help

collection area of solar water heater? given energy of sunlight in kj and how much to install given price/m2?

The average home has a 200 liter (50-60 gallon) hot-water tank, which is effectively drained and replenished three times per day. Assume that the entering tap water is 19 degrees C and is heated to 51 degrees C. Given an average energy from sunlight of 1.53 kJ/cm2 per day, how large would the collection area (in m2) of a solar water heater need to be if its efficiency is 26%? Assume that the price of a solar collector is $375/m2. How much would it cost to install this hot water system? I don't know where to begin on this. Please give me the answers and formulas used.

given concentrations in molec/cm3 and ppm, calculate rate of reaction given rate constant

For the concentration of hydroxyl radical of 7.5E06 molecules/cm3 and a carbon monoxide concentration of 18 ppm, calculate the rate of its reaction with atmospheric carbon monoxide at 11 degrees C, given that the rate constant for the process is 5E-13 E-300/T molecule-1 cm3 sec-1. Hint: Convert the rate constant to a numerical value. Calculate the CO concentration to molecules/cm3, calculate the rate. I can't seem to find what T means. Please need the right ANSWER and formulas...