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2 years ago

Please help me with number 4 and 5 on my study guide

Chemistry

1 answer:

Shtirlitz [24]2 years ago

5 0

Answer:

help with problem 4

Explanation:

4. protons are equal to atomic numbers. neutrons are atomic mass minus atomic number. electrons are equal to protons.

5. I don't know, sorry.

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Hello. I have a new science test and I’m checking my answers. I would like some help.

Burka [1]

Answer:

1. D. Boat B will cause a change in the position and speed of boat A.

2. B. A collision

3. D.

4. Most likely C

Explanation:

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3 years ago

What effect does the addition of a catalyst have on a chemical reaction at equilibrium?

svetlana [45]

Answer:

Explanation:

In the presence of a catalyst, both the forward and reverse reaction rates will speed up equally. :)

7 0

3 years ago

A sample of propane (C3H8) is placed in a closed vessel together with an amount of O2 that is 3 times the amount needed to compl

Aneli [31]

Answer:

final mole fraction of O₂ = 58.84% , CO₂ = 17.64% , H₂O = 23.52% .

final partial pressure of O₂ = 2.942 atm , CO₂ = 0.882 atm , H₂O = 1.176 atm .

Explanation:

Assuming that propane is present as a gas , and also that the combustion is complete:

C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O

then taking as a reference propane sample= 1 mol , then

initial moles of O₂ = 3* 5 moles = 15 moles

final moles of O₂= 3* 5 moles - 5 moles = 10 moles

final moles of CO₂ = 3 moles

final moles of H₂O = 4 moles

total number of moles = 10 + 3 + 4 = 17 moles

final mole fraction of O₂ = 10/17 = 0.5884 = 58.84%

final mole fraction of CO₂ = 3/17 = 0.1764 = 17.64%

final mole fraction of H₂O = 4/17 = 0.2352 = 23.52%

From Dalton's law for ideal gases , the partial pressure p=P*x then

final partial pressure of O₂ = 5 atm * 10/17 = 2.942 atm

final partial pressure of CO₂ = 5 atm * 3/17 = 0.882 atm

final partial pressure of H₂O = 5 atm * 1/17 = 1.176 atm

4 0

3 years ago

Read 2 more answers

Solve the equation for n 0.0092=0.608 x (n/84.01)+n/52.5

kotegsom [21]

Answer:

$n\approx 0.350$

Explanation:

1. Rewrite the equation in a more appropriate format for a better understanding:

$0.0092=0.608\times \dfrac{n}{84.01}+\dfrac{n}{52.5}$

2. Multiply the whole equation (both sides) by 84.01 × 52.5 to eliminate the denominators:

$0.0092\times 84.01\times 52.5=0.608\times 52.5n+84.01n$

3. Do the operations:

$40.57683=31.92n+84.01n$

4. Add like terms:

$40.57683=115.93n$

5. Divide both sides by 115.93:

$0.350011\approx n\\\\n\approx 0.350011\\\\n\approx 0.350$

3 0

4 years ago

A fuel-air mixture is placed in a cylinder fitted with a piston. The original volume is 0.310-L. When the mixture is ignited, ga

Soloha48 [4]

Answer:

$V_2=11.35L$

Explanation:

Knowing that the system is at constant pressure, the energy balance is:

$\Delta H=Q-W$

If all the energy (enthalpy of combustion) is transformed into work:

$\Delta H=-W$

Work:

$W=-\int_{V1}^{V2}P*dV$

$W=-P*(V_2-V_1)$

$\Delta H=P*(V_2-V_1)$

Calculating:

$935J=84659 Pa*(V_2-3.1*10^{-4}m^3)$

$V_2=0.0113 m^3=11.35L$

3 0

3 years ago