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Ksivusya [100]
3 years ago
11

What are examples of inferred energy?

Chemistry
2 answers:
Kisachek [45]3 years ago
6 0
Using a stove to heat up water.  
beks73 [17]3 years ago
3 0
When your hair is really wet so you have to use a hairdryer
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Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g) Which half reaction correctly describes the oxidation that is taking place?
abruzzese [7]
Zn (s) -> Zn+2 (aq) + 2e-

Zn (s) with a neutral charge is oxidized and looses two electrons in the process to form ZnCl2 (aq) where Zn has a charge of 2+.
8 0
3 years ago
Read 2 more answers
Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order in HI, and the rate constant is 9.7×10−6M−
Lady bird [3.3K]

Answer : The molarity after a reaction time of 5.00 days is, 0.109 M

Explanation :

The integrated rate law equation for second order reaction follows:

k=\frac{1}{t}\left (\frac{1}{[A]}-\frac{1}{[A]_o}\right)

where,

k = rate constant = 9.7\times 10^{-6}M^{-1}s^{-1}

t = time taken  = 5.00 days

[A] = concentration of substance after time 't' = ?

[A]_o = Initial concentration = 0.110 M

Now put all the given values in above equation, we get:

9.7\times 10^{-6}=\frac{1}{5.00}\left (\frac{1}{[A]}-\frac{1}{(0.110)}\right)

[A]=0.109M

Hence, the molarity after a reaction time of 5.00 days is, 0.109 M

8 0
3 years ago
4. What is the role of the<br> benedict solution in testing for<br> presence of carbohydrates
Vanyuwa [196]

Answer:

it identifies reducing sugars (monosaccharide's and some disaccharides), which have free ketone or aldehyde functional group

Explanation:

It turns from turquoise to yellow or orange when it reacts with reducing sugars.

3 0
2 years ago
Determine the number of grams of Carbon in 215 g of sucrose.
olya-2409 [2.1K]
<span>just find the percent mass of oxygen in sucrose again. and then multiply that by 50.00.</span>
6 0
3 years ago
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation:
rusak2 [61]

Answer:

60.42% is the percent yield of the reaction.

Explanation:

Moles of methane gas at 734 Torr and a temperature of 25 °C.

Volume of methane gas = V = 26.0 L

Pressure of the methane gas = P = 734 Torr = 0.9542 atm

Temperature of the methane gas = T = 25 °C = 298.15 K

Moles of methane gas = n

PV=nRT

n=\frac{PV}{RT}=\frac{0.9542 atm\times 26.0L}{0.0821 atm L/mol K\times 298.15 K}=1.0135 mol

Moles of water vapors at 700 Torr and a temperature of 125 °C.

Volume of water vapor = V' = 23.0 L

Pressure of water vapor = P' = 700 Torr = 0.9100 atm

Temperature of  water vapor = T' = 125 °C = 398.15 K

Moles of water vapor gas = n'

P'V'=n'RT'

n'=\frac{PV}{RT}=\frac{0.9100 atm\times 23.0L}{0.0821 atm L/mol K\times 398.15 K}=0.6402 mol

CH_4(g)+H_2O(g)\rightarrow CO(g)+3H_2(g)

According to reaction , 1 mol of methane reacts with 1 mol of water vapor. As we can see that moles of water vapors are in lessor amount which means it is a limiting reagent and formation of hydrogen gas will depend upon moles of water vapors.

According to reaction 1 mol of water vapor gives 3 moles of hydrogen gas.

Then 0.6402 moles of water vapor will give:

\frac{3}{1}\times 0.6402 mol=1.9208 mol of hydrogen gas

Moles of hydrogen gas obtained theoretically = 1.9208 mol

The reaction produces 26.0 L of hydrogen gas measured at STP.

At STP, 1 mole of gas occupies 22.4 L of volume.

Then 26 L of volume of gas will be occupied by:

\frac{1}{22.4 L}\times 26 L= 1.1607 mol

Moles of hydrogen gas obtained experimentally = 1.1607 mol

Percentage yield of hydrogen gas of the reaction:

\frac{Experimental}{Theoretical}\times 100

\%=\frac{ 1.1607 mol}{1.9208 mol}\times 100=60.42\%

60.42% is the percent yield of the reaction.

8 0
3 years ago
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