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hodyreva [135]
2 years ago
13

Consider the energy transfers and transformations that occur when a person rides a bicycle. Describe thi

Chemistry
2 answers:
Leno4ka [110]2 years ago
8 0

Answer:

b,a,b

Explanation:

cupoosta [38]2 years ago
7 0

Answer:

1.B

2.A

3.B

Explanation:

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1. 2Na + 2HCl --> 2NaCl + H2
snow_tiger [21]

Answer:

                 

Explanation:

4 0
2 years ago
Read 2 more answers
A solution that is a 4 on pH scale is a
Dominik [7]
A pH scale runs from 1 to 14 with 7 being neutral.

1-6 has base like properties
8-14 has avid line properties

since this solution has a pH scale of 4.... the solution is basic
3 0
3 years ago
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In acidic solution, the sulfate ion can be used to react with a number of metal ions. One such reaction is SO42−(aq)+Sn2+(aq)→H2
allsm [11]

Answer:

The final balanced equation is :

SO_4^{2-}(aq)+4H^+(aq)+Sn^{2+}(aq)\rightarrow H_2SO_3(aq)+H_2O(l)+Sn^{4+}(aq)

Explanation:

SO_4^{2-}(aq)+Sn^{2+}(aq)\rightarrow H_2SO_3(aq)+Sn^{4+}(aq)

Balancing in acidic medium:

First we will determine the oxidation and reduction reaction from the givne reaction :

Oxidation:

Sn^{2+}(aq)\rightarrow Sn^{4+}(aq)

Balance the charge by adding 2 electrons on product side:

Sn^{2+}(aq)\rightarrow Sn^{4+}(aq)+2e^-....[1]

Reduction :

SO_4^{2-}(aq)\rightarrow H_2SO_3(aq)

Balance O by adding water on required side:

SO_4^{2-}(aq)\rightarrow H_2SO_3(aq)+H_2O(l)

Now, balance H by adding H^+ on the required side:

SO_4^{2-}(aq)+4H^+(aq)\rightarrow H_2SO_3(aq)+H_2O(l)

At last balance the charge by adding electrons on the side where positive charge is more:

SO_4^{2-}(aq)+4H^+(aq)+2e^-\rightarrow H_2SO_3(aq)+H_2O(l)..[2]

Adding [1] and [2]:

SO_4^{2-}(aq)+4H^+(aq)+Sn^{2+}(aq)\rightarrow H_2SO_3(aq)+H_2O(l)+Sn^{4+}(aq)

The final balanced equation is :

SO_4^{2-}(aq)+4H^+(aq)+Sn^{2+}(aq)\rightarrow H_2SO_3(aq)+H_2O(l)+Sn^{4+}(aq)

4 0
3 years ago
Calculate the partial pressure of oxygen given the total barometric pressure of 515 mmHg. Round to the nearest hundredth.
Eva8 [605]

The partial pressure of oxygen given the total barometric pressure is : 108.15 mmHg

<u>Given data : </u>

Total barometric pressure = 515 mmHg

Assuming oxygen percentage = 21%

Barometric pressure dry at 37°C

<h3 /><h3>Determine the partial pressure of oxygen </h3>

Applying  the relation below

Partial pressure = oxygen percentage * Barometric pressure

                          = 21% * 515 mmHg

                          = 108.15 mmHg

Hence we can conclude that the partial pressure of oxygen is 108.15 mmHg.

Learn more about Partial pressure : brainly.com/question/1835226

8 0
2 years ago
Complete combustion of 8.10 g of a hydrocarbon produced 25.9 g of CO2 and 9.27 g of H2O. What is the empirical formula for the h
balu736 [363]

CxHy     +  O2    -->    x CO2     +    y/2  H2O

 

Find the moles of CO2 :     18.9g  /  44 g/mol   =    .430 mol CO2   = .430 mol of C in compound

Find the moles of H2O:      5.79g / 18 g/mol     =     .322 mol H2O   = .166 mol of H in compound

 

Find the mass of C and H in the compound:

                             .430mol  x 12  =  5.16 g C

                              .166mol  x 1g   = .166g H   

 

When you add these up they indicate a mass of 5.33 g for the compound, not 5.80g as you stated in the problem.

Therefore it is likely that either the mass of the CO2 or the mass of H20 produced is incorrect (most likely a typo).

In any event, to find the formula, you would take the moles of C and H and convert to a whole number ratio (this is usually done by dividing both of them by the smaller value).

8 0
3 years ago
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