When one gram of gas, is burned, 55.5kJ of heat are released. How many pounds of methane gas must be burned to release 2.578 x 10^3kJ of heat?
CH4 + 2O2 ==> CO2 + 2H2O + heat
So you get 55.5 kJ for 1 gram CH4.
You want how many grams to produce 2578 kJ.
1 gram x (2578/55.5) = ? grams CH4 required. Convert that to pounds.
To solve this problem, we need to convert between grams and pounds.
Step 1: Convert grams to pounds
There are 454 grams in a pound. Therefore, we can convert grams to pounds by dividing the number of grams by 454.
Step 2: Calculate the number of pounds of methane gas
Let's assume x is the number of pounds of methane gas that must be burned to release 2.578 x 10^3 kJ of heat.
Using the given information, we can establish a proportion:
1 gram of gas / 55.5 kJ = x pounds of gas / 2.578 x 10^3 kJ
Cross-multiply and solve for x:
1 * (2.578 x 10^3) kJ = 55.5 kJ * x
2.578 x 10^3 kJ = 55.5 kJ * x
Divide both sides by 55.5 kJ to isolate x:
(2.578 x 10^3 kJ) / 55.5 kJ = (55.5 kJ * x) / 55.5 kJ
x = (2.578 x 10^3 kJ) / 55.5 kJ
Step 3: Perform the calculation
x = 46.4864864865
Therefore, approximately 46.49 pounds of methane gas must be burned to release 2.578 x 10^3 kJ of heat.