Answer:
Pb(NO3)2(aq) + 2NaCl(aq) —> PbCl2(s) + 2NaNO3(aq)
Explanation:
When lead (II) nitrate, Pb(NO3)2 undergoes a double displacement reaction with aqueous sodium chloride, NaCl, the following products are obtained:
Pb(NO3)2(aq) + NaCl(aq) —>
Aqueous Pb(NO3)2 will dissociate in solution as follow:
Pb(NO3)2(aq) —> Pb2+(aq) + 2NO3-(aq)
On the other hand, aqueous NaCl will dissociate as follow:
NaCl(aq) —> Na+(aq) + Cl-(aq)
The double displacement reaction will take place as follow:
Pb(NO3)2(aq) + NaCl(aq) —>
Pb2+(aq) + 2NO3-(aq) + Na+(aq) + Cl-(aq) —> Pb2+(aq) Cl-(aq) + Na+(aq) 2NO3-(aq)
Pb(NO3)2(aq) + NaCl(aq) —> PbCl2(s) + NaNO3(aq)
We simply balance the equation by putting 2 in front of NaCl and 2 in front of NaNO3 as shown below:
Pb(NO3)2(aq) + 2NaCl(aq) —> PbCl2(s) + 2NaNO3(aq)
Tetraphosphorus Decaoxide has a molecular formula of P4O10,
all else are known. Therefore the balanced chemical equation would be:
4PH3 + 8O2 --> 6H2O + P4O10
Taking into account the phases:
4PH3(g) + 8O2(g) --> 6H2O(g) + P4O10(s)
Answer:
[OH-] = 1.08x10^-11 M
Explanation:
From the question given,
Concentration of Hydrogen ion, [H+]
= 9.3x10^-4 M
Concentration of Hydroxide ion, [OH-] =..?
The concentration of the hydrogen ion, [H+] and hydroxide ion, [OH-] are related with the following formula:
[H+] x [OH-] = 1x10^-14
Using the above formula, we can easily calculate the concentration of the hydroxide ion, [OH-] as follow:
[H+] x [OH-] = 1x10^-14
[H+] = 9.3x10^-4 M
9.3x10^-4 x [OH-] = 1x10^-14
Divide both side by 9.3x10^-4
[OH-] = 1x10^-14 /9.3x10^-4
[OH-] = 1.08x10^-11 M
Answer:
The answer would be C. 1852.3
Explanation:
<u>Answer:</u> The partial pressure of carbon dioxide is 858 torr
<u>Explanation:</u>
Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.
To calculate the partial pressure of hydrogen gas, we use the law given by Dalton, which is:
We are given:
Total pressure of the carbonated drink, = 890 torr
Vapor pressure of water, = 32 torr
Putting values in above equation, we get:
Hence, the partial pressure of carbon dioxide is 858 torr.