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s344n2d4d5 [400]
3 years ago
14

You are given 230 grams of a substance with a half-life of 0.75 years. How much will remain after 3 years?

Chemistry
1 answer:
Degger [83]3 years ago
6 0
After 3 years, the substance will go through 4 half lives. You can do 230*(1/2)^4, which is 14.375.
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Yes..? I don’t understand what you’re trying to ask mate.
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3 years ago
Water has a high specific heat because: Select one: a. it is a poor insulator b. hydrogen bonds must be broken to raise its temp
Crank
<h2>The required "option is b) hydrogen bonds must be broken to raise its temperature.</h2>

Explanation:

  • Water has high specific heat due to hydrogen bonds present in it.
  • The Ionisation of water does not affect the specific heat of the water.
  • On decreasing the temperature, there is the formation of bonds hence option (d) is wrong.
  • On increasing the temperature, there is the breaking of bonds hence option (b) is correct.
3 0
3 years ago
How many atoms are present in 65.39 g of zinc?
klio [65]
<span>Avogadro's number represents the number of units in one mole of any substance. This has the value of 6.022 x 10^23 units / mole. This number can be used to convert the number of atoms or molecules into number of moles.

 65.39 g Zn ( 1 mol / 65.38 g ) ( </span>6.022 x 10^23 atoms / 1 mol ) = 6.023x10^23 atoms Zn
3 0
3 years ago
One of the reactions that occurs in a blast furnace, in which iron ore is converted to cast iron, is Fe2O3 + 3CO → 2Fe + 3CO2 Su
Tpy6a [65]

Answer : The percent purity of Fe_2O_3 in the original sample is 87.94 %

Explanation :

The given balanced chemical reaction is:

Fe_2O3+3CO\rightarrow 2Fe+3CO_2

First we have to calculate the mass of Fe.

\text{Moles of }Fe=\frac{\text{Mass of }Fe}{\text{Molar mass of }Fe}

Molar mass of Fe = 55.8 g/mole

\text{Moles of }Fe=\frac{1.79\times 10^3kg}{55.8g/mole}=\frac{1.79\times 10^3\times 1000g}{55.8g/mole}=3.15\times 10^4mole

Now we have to calculate the moles of Fe_2O_3

From the balanced chemical reaction we conclude that,

As, 2 moles of Fe produced from 1 mole of Fe_2O_3

So, 3.15\times 10^4mole of Fe produced from \frac{3.15\times 10^4}{2}=15750 mole of Fe_2O_3

Now we have to calculate the mass of Fe_2O_3

\text{ Mass of }Fe_2O_3=\text{ Moles of }Fe_2O_3\times \text{ Molar mass of }Fe_2O_3

Molar mass of Fe_2O_3 = 159.69 g/mole

\text{ Mass of }Fe_2O_3=(15750moles)\times (159.69g/mole)=2.515\times 10^6g=2.515\times 10^3kg

Now we have to calculate the percent purity of Fe_2O_3 in the original sample.

Mass of original sample = 2.86\times 10^3kg

\text{Percent purity}=\frac{\text{Mass of }Fe_2O_3}{\text{Mass of sample}}\times 100

\text{Percent purity}=\frac{2.515\times 10^3kg}{2.86\times 10^3kg}\times 100=87.94\%

Therefore, the percent purity of Fe_2O_3 in the original sample is 87.94 %

3 0
3 years ago
What is the redox equation for sulphuric acid and magnesium ribbon
Wewaii [24]
Sulfuric acid: H_2SO_4_{(aq)}
Magnesium ribbon: Mg_(s)
Mg_{(s)}+H_2SO_4_{(aq)} \rightarrow MgSO_4_{(aq)}+H_2_{(g)}
8 0
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