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vlada-n [284]
3 years ago
10

What are the oxidation numbers of the elements in the nitrite ion, no2−?

Chemistry
1 answer:
sdas [7]3 years ago
8 0
N = 3
O = -2
1(3) +2(-2)= -1

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How many grams of salt are in 1 kilogram of seawater with average salinity? quizzlet?
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State Boyle's, Charles's, and Gay-Lussac's laws using sentences, then equations
dimaraw [331]

Explanation:

1. Boyle's Law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

P\propto \frac{1}{V}      (At constant temperature and number of moles)

P_1\times {V_1}=P_2\times V_2

2. Charles' Law states that volume is directly proportional to the temperature of the gas at constant pressure and number of moles.

V\propto T    (At constant pressure and number of moles

\frac{V_1}{T_1}=\frac{V_2}{T_2}

3. Gay Lussac's Law states that tempertaure is directly proportional to the pressure of the gas at constant volume and number of moles of gas

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\frac{V_1}{n_1}=\frac{V_2}{n_2}

7 0
3 years ago
Based on your answers to parts a, b, and c select the best lewis structure (electron-dot structure) for hoi.
vodomira [7]

Answer : The lewis dot structure includes the lone pair of electrons in any element and is helpful for defining the bond formation using the electrons.


In the molecule of HOI hydrogen is to the left of oxygen; oxygen is in middle and Iodine is at right of oxygen.


The picture is attached for better understanding.

6 0
3 years ago
When you put a bottle of juice in a cooler full of ice the juice gets cold that's because the cold transfers to the juice and sl
zubka84 [21]
Because the ice helps cool it up


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3 years ago
Consider the reaction 2CO * O2 —&gt; 2 CO2 what is the percent yield of carbon dioxide (MW= 44g/mol) of the reaction of 10g of c
Arturiano [62]

Answer:

Y = 62.5%

Explanation:

Hello there!

In this case, for the given chemical reaction whereby carbon dioxide is produced in excess oxygen, it is firstly necessary to calculate the theoretical yield of the former throughout the reacted 10 grams of carbon monoxide:

m_{CO_2}^{theoretical}=10gCO*\frac{1molCO}{28gCO}*\frac{2molCO_2}{2molCO}  *\frac{44gCO_2}{1molCO_2}\\\\ m_{CO_2}^{theoretical}=16gCO_2

Finally, given the actual yield of the CO2-product, we can calculate the percent yield as shown below:

Y=\frac{10g}{16g} *100\%\\\\Y=62.5\%

Best regards!

8 0
3 years ago
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