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Svet_ta [14]
2 years ago
12

Can someone show me a step by step with the answer?

Chemistry
1 answer:
Georgia [21]2 years ago
8 0

Answer:

6 mols HCl

Explanation:

(I'm an AP chemistry student but not perfect at this stuff)

you can use the Molarity=Moles/L equation here:

(6M)=(moles HCl)/(1L)

divide by 1 on both sides to isolate the moles of HCl

this gets you 6 moles HCl.

Again I'm just a student so my answer might be wrong, but this question should just require the M=mols/L equation :).

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the gas left in an used aerosol can is at a pressure of 103 kPa at 25 degrees celsius if this can be thrown into fire what is th
Rainbow [258]
Hello!

The pressure of the gas when it's temperature reaches 928 °C is 3823,36 kPa

To solve that we need to apply Gay-Lussac's Law. It states that the pressure of a gas when the volume is left constant (like in the case of a sealed container like an aerosol can) is proportional to temperature. This is the relationship derived from this law that we use to solve this problem:

P2= \frac{P1}{T1}*T2= \frac{103 kPa}{25}*928=3823,36 kPa

Have a nice day!
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3 years ago
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Firdavs [7]

Answer:

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3 years ago
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For each reaction, find the value of ΔSo. Report the value with the appropriate sign. (a) 3 NO2(g) + H2O(l) → 2 HNO3(l) + NO(g)
aev [14]

Answer:

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Explanation:

Let's consider the following balanced equation.

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ni are the moles of reactants and products

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ΔS° = [2 mol × S°(HNO₃(l)) + 1 mol × S°(NO(g))] - [3 mol × S°(NO₂(g)) + 1 mol × S°(H₂O(l))]

ΔS° = [2 mol × 155.6 J/K.mol + 1 mol × 210.76 J/K.mol] - [3 mol × 240.06 J/K.mol + 1 mol × 69.91 J/k.mol]

ΔS° = -268.13 J/K

7 0
3 years ago
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kenny6666 [7]

Answer:

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espero que esto ayude

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3 years ago
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