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3 years ago

What is an isotope? list the isotopes of hydrogen in order from lighter to heavier. which is the most common among them?

1 answer:

6 0

Isotopes= a group of atoms with the same no. of protons , but different no. of neutrons

Hydrogen isotopes

$^1H\implies ^2H\implies ^3H$

The name of the second isotope is deuterium and the name of the third isotope is tritium(radioactive).The most abundant isotope is $^1H$

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a flight stimulator that helps astronauts prepare for a shuttle launch is an example of a (an) ______.

Dimas [21]

A flight simulator that helps astronauts prepare for a shuttle launch is an example of a Scientific Model.

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4 years ago

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Using the activity series, write balanced chemical equations for the following reactions. If not reaction occurs, simply write N

MissTica

Answer:

a) $2 Ni (s) + Cu(NO_3)_2 (aq) \longrightarrow Cu(s) + 2 NiNO_3 (aq)$

b) NR

c) NR

d) $2 Cr (s) + 3 CoCl_2 (aq) \longrightarrow 3 Co(s) + 2CrCl_3 (aq)$

e) NR

Explanation:

a) Nickel is more reactive than copper so the first one will displace the other:

$2 Ni (s) + Cu(NO_3)_2 (aq) \longrightarrow Cu(s) + 2 NiNO_3 (aq)$

b) Due to the higher reactivity the magnesium has compared to the zinc, the first will remain in solution and the second will reamin solid. So, NR.

c) No reaction occurs, gold is resistant to acid in normal conditions due to its characteristic as noble metal.

d) Chromium is more reactive than cobalt so the last one will be displaced:

$2 Cr (s) + 3 CoCl_2 (aq) \longrightarrow 3 Co(s) + 2CrCl_3 (aq)$

e) Nothing happens, the reduction potencial of the hydrogen gas bubbled ins't enough to reduce the silver.

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3 years ago

Calculate ΔHrxn for the following reaction: CH4(g)+2O2(g)→CO2(g)+2H2O(l) Use the following reactions and given ΔH′s. CH4(g)+O2(g

harkovskaia [24]

Answer:

ΔH of CH4(g)+2O2(g)→CO2(g)+2H2O(l) is -899 KJ

Explanation:

step 1: write down thye reaction and rearrange them in a way that similar contents cancel out to produce the required reaction and add the enthalpy change of each.

CH4(g)+O2(g)→CH2O(g)+H2O(g) ΔH = -284 KJ

CH2O(g)+O2(g)→CO2(g)+H2O(g) ΔH = -527 KJ

2H2O(g)→2H2O(l) ΔH = 44 KJ x -2

the minus is because the last reaction has been reversed and multiplied by 2 so that the gaseous state H2O cancels with the others to leave liquid H2O in the required final reaction.

ΔHrxn = (-284)+(-527)+[44 x (-2)] = -899 KJ

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3 years ago

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1. How many molecules of ammonia can be created when four molecules of nitrogen are combined with four molecules of hydrogen? In

allochka39001 [22]

Explanation:

1. $N_2+3H_2\rightarrow 2NH_3$

According to reaction , 1 molecule of nitrogen gas reacts with 3 molecules of hydrogen gas to give 2 molecules of ammonia

Then 4 molecules of nitrogen gas will react with:

$\frac{3}{1}\times 4 molecules=12 molecules$ of hydrogen gas.

As we can see that molecules of nitrogen gas are in excess amount.

So, the molecules of ammonia formed will depend upon molecules of hydrogen gas.

According to reaction, 3 molecules of hydrogen gas gives 2 molecules of ammonia.

Then 4 molecules of hydrogen gas will give :

= $\frac{2}{3}\times 4 molecules=2.667 molecules$ of ammonia

2) $N_2+3H_2\rightarrow 2NH_3$

Molecules of nitrogen gas in balanced chemical equation = 1

Molecules of hydrogen gas in balanced chemical equation = 3

The ratio of nitrogen and hydrogen molecules would result in no left-over reactants will be:

$\frac{1}{3}$ = 1 : 3

For every 1 molecule of nitrogen gas molecules 3 molecules of hydrogen gas molecules are required to form.

3) $N_2+3H_2\rightarrow 2NH_3$

Moles of nitrogen gas = $\frac{100.0 g}{28 g/mol}=3.5714 mol$

Moles of hydrogen gas = $\frac{100.0 g}{2 g/mol}=50.0 mol$

According to reaction , 1 mole of nitrogen gas reacts with 3 mole of hydrogen gas to give 2 moles of ammonia

Then 3.5714 moles of nitrogen gas will react with:

$\frac{3}{1}\times 3.5714 mol=10.7142 mol$ of hydrogen gas.

As we can see that moles of nitrogen gas are only reacting with 10.7142 moles of hydrogen gas which means that nitrogen gas is limiting reagent and hydrogen gas is excessive reagent.

So, amount of ammonia gas will depend upon the moles of nitrogen gas.

According to reaction, 1 molecules of nitrogen gas gives 2 molecules of ammonia.

Then 3.5714 mol of nitrogen gas will give :

= $\frac{2}{1}\times 3.5714 mol=7.1428 mol$ of ammonia