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Artemon [7]
3 years ago
14

1. What is the weight of the ethyl alcohol that exactly fills a 200.0 mL container? The density of ethyl alcohol is 0.789 g/mL

Chemistry
1 answer:
timofeeve [1]3 years ago
3 0
Multiply 0.789g/mL by 200.0mL to obtain 157.8g of ethyl alchohol to fill the entire container.
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Which of the following displays the correct change in enthalpy and best describes the reaction below? 2CsCl(aq) + Na2SO4(aq) 2Na
Bond [772]
We subtract the enthalpies of the reactants from that of the products:
2\Delta
 H(NaCl)+\Delta H(Cs_2 SO_4)-2\Delta H(CsCl)-\Delta H(Na_2 SO_4) \\ 
=2(-411)+(-1400) -2(-415)-(-1380) \\ = -12 kJ
Since this is < 0, this is an exothermic reaction.

3 0
3 years ago
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Explanation:

4 0
3 years ago
How many moles of NH3 can you make from 6.20 moles of N2?
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4 0
3 years ago
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If 20 grams of Zinc phosphate reacts with excess hydrochloric acid and produces 18 grams of Zinc chloride what is the percent yi
fenix001 [56]

Answer:

Y=85\%

Explanation:

Hello!

In this case, since we know the balanced chemical reaction, we are first able to realize there is a 1:3 mole ratio between zinc phosphate and zinc chloride; it means that we can first compute the moles of the desired product via stoichiometry:

n_{ZnCl_2}=20gZn_3(PO_4)_2*\frac{1molZn_3(PO_4)_2}{386.11gZn_3(PO_4)_2}*\frac{3molZnCl_2}{1molZn_3(PO_4)_2}=0.16gZnCl_2

Next, since those moles are associated with the theoretical yield of zinc chloride, we obtain the corresponding mass:

m_{ZnCl_2}^{theoretical}=0.16molZnCl_2*\frac{136.29gZnCl_2}{1molZnCl_2} =21gZnCl_2

Finally, we compute the percent yield by diving the actual yield (18 g) by the theoretical yield:

Y=\frac{18g}{21g}*100\%\\\\Y=85\%

Best regards!

4 0
3 years ago
How many grams are in a 1.48x107 ig
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Answer:978989989.1429323

Explanation:

6 0
2 years ago
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