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1 year ago

Help me with this question please

Chemistry

1 answer:

mash [69]1 year ago

6 0

Answer:

a. Oxidising agent: Cl₂

b. Reducing agent: NaBr

c. Oxidised: NaBr

d. Reduced: Cl₂

e. Oxidation numbers before reaction: Cl= 0, Na= +1, Br= -1

f. Oxidation numbers after reaction: Cl= -1, Na= +1, Br= 0

Explanation:

Oxidising agents reduces themselves, oxidising other elements/compounds.

Reducing agents oxidise themselves, reducing other elements/compounds.

Oxidation is the loss of electrons or an increase in oxidation number.

Reduction is the gain of electrons or decrease in oxidation number.

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Each molecule of table sugar, C12H22O11, contains

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D, because C12 means there's 12 atoms of carbon.

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An ion is formed when an atom___?

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gain or loses electrons.

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3 years ago

Aluminum reacts with sulfur gas to produce aluminum sulfide. a) What is the limiting reactant? What is the excess reagent? b) Ho

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Answer:

a) Limiting: sulfur. Excess: aluminium.

b) 1.56g Al₂S₃.

c) 0.72g Al

Explanation:

Hello,

In this case, the initial mass of both aluminium and sulfur are missing, therefore, one could assume they are 1.00 g for each one. Thus, by considering the undergoing chemical reaction turns out:

$2Al(s)+3S_2(g)\rightarrow 2Al_2S_3(s)\\$

a) Thus, considering the assumed mass (which could be changed based on the one you are given), the limiting reagent is identified as shown below:

$n_S^{available}=1.00gS_2*\frac{1molS_2}{64gS_2} =0.0156molS_2\\n_S^{consumed\ by \ Al}=1.00gAl*\frac{1molAl}{27gAl}*\frac{3molS_2}{2molAl}=0.0556molS_2$

Thereby, since there 1.00g of aluminium will consume 0.0554 mol of sulfur but there are just 0.0156 mol available, the limiting reagent is sulfur and the excess reagent is aluminium.

b) By stoichiometry, the produced grams of aluminium sulfide are:

$m_{Al_2S_3}=0.0156molS_2*\frac{2molAl_2S_3}{3molS_2} *\frac{150gAl_2S_3}{1molAl_2S_3} =1.56gAl_2S_3$

c) The leftover is computed as follows:

$m_{Al}^{excess}=(0.0556-0.0156)molS_2*\frac{2molAl}{3molS_2}*\frac{27gAl}{1molAl} =0.72 gAl\\$

NOTE: Remember I assumed the quantities, they could change based on those you are given, so the results might be different, but the procedure is quite the same.

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3 years ago

How does the type of liquid used to make ice cubes affect the rate at which it melts?

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Liquid water can be separated into hydrogen gas and oxygen gas through electrolysis. 1 mole of hydrogen gas and 0.5 moles of oxy

soldier1979 [14.2K]

The temperatures of the gases will not be equal as oxygen gas will have a higher temperature than hydrogen gas because it has fewer moles overall.

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The mechanical behavior of ideal gases is described by the ideal gas law. It has the ability to compute the volume of gases created or absorbed.

This equation is frequently used in chemical equations to convert between volumes and molar quantities.

According to the ideal gas law, there is a relationship between gas pressure, temperature, and volume.

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T is same for both.

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1 year ago