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fiasKO [112]
3 years ago
7

Look at the image shown.

Chemistry
1 answer:
Charra [1.4K]3 years ago
6 0
Where’s the image sorry this isn’t much help but I don’t know what to answer if I can’t see the image
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What is the balanced chemical equation for the reaction of aqueous sodium hydroxide and sulfuric acid?
Andrews [41]

Answer:

H2SO4 + 2(NaOH) -----> Na2SO4 + 2(H2O).

Explanation:

6 0
3 years ago
You have a cold and symptoms include a runny nose, fever and coughing. How is your body working together to get rid of the bacte
topjm [15]
Your white blood cells are fighting the pathogen (sickness)
8 0
4 years ago
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The reaction          3 BrO- (aq) --> BrO3- (aq) + 2 Br - (aq) in basic solution is second order in BrO-(aq) with a rate cons
Phoenix [80]

Answer:

0.124 M

Explanation:

The reaction obeys second-order kinetics:

r = k[BrO^-]^2

According to the integrated second-order rate law, we may rewrite the rate law in terms of:

\dfrac{1}{[BrO^-]_t} = kt + \dfrac{1}{[BrO^-]_o}

Here:

k is a rate constant,

[BrO^-]_t is the molarity of the reactant at time t,

[BrO^-]_o is the initial molarity of the reactant.

Converting the time into seconds (since the rate constant has seconds in its units), we obtain:

t = 1.00 min = 60.0 s

Rearranging the integrated equation for the amount at time t:

[BrO^-]_t = \dfrac{1}{kt + \dfrac{1}{[BrO^-]_o}}

We may now substitute the data:

[BrO^-]_t = \dfrac{1}{0.056 M^{-1}s^{-1}\cdot 60.0 s + \dfrac{1}{0.212 M}} = 0.124 M

7 0
4 years ago
1.When a driver touches a car's steering wheel on a hot day, heart is transferred to the driver's hands by____.
marin [14]
I think the answer is
B,c,b,d,d,
5 0
3 years ago
Read 2 more answers
calculate the mass of 120cc nitrogen present at STP. how many number of molecules are present in it?​
Stells [14]

Answer:

0.15008\ \text{g}

3.23\times 10^{21}

Explanation:

1 mol of nitrogen at STP = 22.4 L = 22400 cc

n = Mol of N_2 = \dfrac{120}{22400}=0.00536\ \text{mol}

M = Molar mass of N_2 = 28\ \text{g/mol}

N_A = Avogadro's number = 6.022\times 10^{23}\ \text{mol}^{-1}

Mass of N_2 is

m=nM\\\Rightarrow m=0.00536\times 28\\\Rightarrow m=0.15008\ \text{g}

Mass of the nitrogen is 0.15008\ \text{g}

Number of molecules is given by

nN_A=0.00536\times 6.022\times 10^{23}=3.23\times 10^{21}\ \text{molecules}

The number of molecules present in it are 3.23\times 10^{21}

5 0
3 years ago
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