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butalik [34]
3 years ago
15

the half-life of chromium 51 is 28 days if the sample contained 510 grams how much chromium would remain after 86 days​

Chemistry
1 answer:
Anni [7]3 years ago
5 0

Answer: 3.285714285714286 I believe this is what it is

Explanation:

You have to divide 50 by 28 then times it by 510 then divide by 86

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Answer:

The heat released is 56.7 kJ.

Explanation:

To solve this problem, first we need to find out the standard enthalpy of reaction, that is, the energy released at constant pressure in standard conditions (P=1bar, T=298.15K). We can find it using the expression:

ΔH°r = Σn(p).ΔH°f(p) - Σn(r).ΔH°f(r)

where,

n refers to the number of moles of reactants and products in the balanced equation

ΔH°f refers to standard enthalpies of formation (which can be found in tables).

Given the equation:

2 H₂O₂(l) → 2 H₂O(g) + O₂(g)

We can replace with the proper data in the equation:

ΔH°r = Σn(p).ΔH°f(p) - Σn(r).ΔH°f(r)

ΔH°r= [2 mol . ΔH°f H₂O(g) + 1 mol . ΔH°f O₂(g)] - [2 mol .  ΔH°f H₂O₂(l)]

ΔH°r= [2 mol . (-241.8 kJ/mol) + 1 mol . 0 kJ/mol] - [2 mol . (-187.8 kJ/mol)]

ΔH°r = -108.0 kJ

Since enthalpy is an extensive property, it depends on the amount of reagents. In this case, 108.0 kJ of heat are released every 2 moles of H₂O₂(l) decomposed. Then, for 1.05 mol of H₂O₂(l):

1.05 mol.\frac{-108.0kJ}{2mol} =-56.7kJ

By convention, the negative sign means that heat is released.

5 0
2 years ago
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