The amount of heat needed to cook the pork roast is 1700 kJ.
The amount of heat absorbed by the roast is 14% of the heat produced = 14% X ?H = 310.38 kJ/mol
One mole of propane burns to produce 3 moles of CO2 and -2217 kJ of heat.
1700kJ/ (14% X ?H) = mol of C3H8 burned
1700kJ / (310.38 kJ/mol) = 5.48 mol C3H8
Since 3 moles of CO2 are produced:
3 X 5.48 mol= 16.43 mols of CO2
convert moles to grams:
16.43 mol CO2 X 44.0g/mol ~ 722.9 g CO2 produced
Answer: (129.12 ft^2) / (24 ft^2/can) = 5.38 cans. Round this up to 6 cans. Please undrstand that this is only an example, since I do not know the actual dimenions of the wall
I dont understand the question
Answer: 3x
Step-by-step explanation:
Answer:
To quickly solve this problem, we can use a graphing tool or a calculator to plot the equation.
Please see the attached image below, to find more information about the graph
The equation is:
y = tan(2x - π)
y = tan (2*(x-π/2))
We can compare it to its parent function
g(x) = tan(x)
The answer is
Option a.
Horizontal shrink by 1/2 and horizontal shift of π/2 to the right
