Answer:
<h2>377 kPa</h2>
Explanation:
The original pressure can be found by using the formula for Boyle's law which is
where
P1 is the initial pressure
P2 is the final pressure
V1 is the initial volume
V2 is the final volume
Since we're finding the original pressure
150 kPa = 150,000 Pa
We have
We have the final answer as
<h3>377 kPa</h3>
Hope this helps you
Answer:
The answer to your question is below
Explanation:
5) Fe₂O₃(s) + 3H₂O ⇒ 2Fe(OH)₃ (ac) Synthesis reaction
6) 2C₄H₁₀(g) + 13O₂(g) ⇒ 8CO₂ (g) + 10H₂O Combustion reaction
7) 2NO₂ (g) ⇒ 2O₂ (g) + N₂ (g) Decomposition reaction
8) H₃P (g) + 2O₂ (g) ⇒ PO (g) + 3H₂O Single replacement reaction
A graph shows a relationship between two variables: independent and dependent. The dependent variable is in the y-axis, while the independent variable is in the x-axis. When it says, plot velocity against time, that means that
velocity is in the y-axis in meters per second, and time is in the x-axis in seconds. An example of a velocity vs time graph is shown in the attached picture. In this example, the motion is in constant acceleration. This is because it is linear, thereby, the slope is constant. If you want to find the instantaneous velocity at a certain time, create a vertical line from the x-axis until it reaches the diagonal line. Then, draw a horizontal line towards the y-axis to know the value of the velocity.
Answer:
0.641 moles of ethane
Explanation:
Based on the equation:
C2H6(g) + 7/2O2(g) → 2CO2(g) + 3H2O(l)
We can determine ΔH of reaction using Hess's law. For this equation:
<em>Hess's law: ΔH products - ΔH reactants</em>
ΔH = {2ΔHCO2 + 3ΔHH2O} - {ΔHC2H6}
<em>Pure monoatomic substances have a ΔH = 0kJ/mol; ΔHO2 = 0kJ/mol</em>
<em />
ΔH = {2*-393.5kJ/mol + 3*-285.8kJ/mol} - {-84.7kJ/mol}
ΔH = -1559.7kJ/mol
That means when 1 mole of ethane is in combustion there are released 1559.7kJ of heat. To produce 1.00x10³kJ there are needed:
1.00x10³kJ * (1mole ethane / 1559.7kJ) =
<h3>0.641 moles of ethane</h3>
