Answer:
1. The balanced thermochemical equation for the reaction is;
2C4H10 (g) + 13O2 (g) -----------> 8CO2 (g) + 10H20 (g)
2. Heat when 200g of butane is burned is 9925.65 kJ of heat
Explanation:
2 moles of butane reacts with oxygen in excess to produce carbon iv oxide and water
If 1 mole releases 2877kJ of heat
2 moles will release (2 * 2877kJ) of heat
= 5754 kJ of heat.
The mass of butane used is 200g and converting it to moles we have;
n = mass / molar mass
molar mass of butane = (12 *4 + 1 *10) = 58 g/mol
So therefore n = 200 g/ 58 g/mol
n= 3.45 moles of butane.
If 1 mole of buatne releases 2877 kJ of heat
3.45 moles will release ( 3.45 * 2877 kJ ) of heat
= 9925.65 kJ of heat
9925.65 kJ of heat is released when 200 g of butane is burned.
Answer:
Explanation:
Hello there!
In this case, according to the given information, it turns out possible for us to calculate the final pressure by using the Boyle's law as an inversely proportional relationship in pressure to volume at constant temperature:
Thus, we solve for our target, P2, to obtain:
Regards!
A simple magnetic compass can be used
Answer:
Explanation:
The density formula is:
Let's rearrange the formula for 
. the volume. Multiply both sides by , then divide by 
.
The volume can be found by dividing the mass by the density. The mass of the object is 30.07 grams and the density is 1.48 grams per milliliter.
Divide. Note, when dividing, the grams, or 
will cancel out.
The volume of the object is 20.317567567568 milliliters.
