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3 years ago

Kinetic energy CANNOT be converted into potential energy True False

Chemistry

2 answers:

Alex777 [14]3 years ago

3 0

Answer:

false

Explanation:

mr Goodwill [35]3 years ago

3 0

Answer:

False

Explanation:

Because if you shoot a arrow and go back and get it and use it again it is potential

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How does a scientist make two solutions with the same molarity? A By dissolving the maximum amount of each substance in the B. B

aalyn [17]

Answer: The answer is “ By dissolving the same number of nmoles of each substance in the same volume of water ”

Explanation:

7 0

4 years ago

consider the reaction between calcium oxide and carbon dioxide: cao ( s ) + co 2 ( g ) → caco 3 ( s ) a chemist allows 14.4 g of

MakcuM [25]

Answer:

CaO is the limiting reagent

Theoritical yield = 25.71 g

% Yield = 75.44%

Explanation:

1 mole = Molar mass of the substance

Molar Mass of CaO = 56 g/mol

Molar Mass of CaCO3 = 100 g/mol

Molar mass of CO2 = 44 g/mol

The balanced Equation is :

$CaO + CO_{2}\rightarrow CaCO_{3}$

1 mole of CaO reacts with = 1 mole of CO2

56 g of CaO reacts with = 44 g of CO2

1 g of CaO reacts with =

$\frac{44}{56}$

= 0.785 g of CO2

So,

14.4 g of CaO must react with = (14.4 x 0.785) g of CO2

= 11.31 g of CO2

Needed = 11.31 g

Available CO2 = 13.8 g (given)

So CO2 is in excess , hence CaO is the limiting reagent and product will produce from 14.4 g of CaO

$CaO + CO_{2}\rightarrow CaCO_{3}$

1 mole of CaO will produce 1 mole pf CaCO3

56 g of CaO produce = 100 g of CaCO3

1 g of CaO produce =

$\frac{100}{56}$

= 1.785 g of CaCO3

14.4 g of CaO will produce = (1.785 x 14.4) g of CaCO3

= 25.71 g of CaCO3

Theoritical Yield of CaCO3 = 25.71 g

Actual yield = 19.4 g

Percent Yield =

$\frac{Actual\ yield}{Theoritical\ yield}\times 100$

$\frac{19.4}{25.71}\times 100$

= 75.44 %

6 0

3 years ago

The burning of propane gas can be represented as a balanced chemical reaction as follows: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Calcula

Snezhnost [94]

Answer: 20L of H2O

Explanation:

C3H8 + 5O2 → 3CO2 + 4H2O

Recall 1mole of a gas contains 22.4L at stp

5moles of O2 contains = 5 x 22.4 = 112L

4moles of H2O contains = 4 x 22.4 = 89.6L

From the equation,

112L of O2 produced 89.6L H2O

There for 25L of O2 will produce XL of H2O i.e

XL of H2O = (25 x 89.6)/112 = 20L

6 0

3 years ago

What the sample will look like after the temperature is increased from 300 K to 450 KK at constant pressure?

sleet_krkn [62]

Answer:

The sample will look expanded and occupy more space.

Explanation:

Since, the pressure is constant here, but the temperature is changed. Therefore, according to Charles' Law Volume is directly proportional to Temperature, provided the pressure is kept constant. Mathematically:

V1/T1 = V2/T2

V1 = (T1/T2)(V2)

V1 = (300 k/450 k)(V2)

V1 = (0.67)V2

The equation indicates that The fina volume of the gas V2 will be greater than the initial volume V1. Thus, sample will look expanded and occupy more space than the previous state.

5 0

3 years ago

Does sound travel best through solids, liquids, or gases?

IRISSAK [1]

In gas the speed of sound is 343.2 meters per second, in liquid the speed of sound is 1,484 meters per second and in solids like steel it travels 5,120 meters per second.

8 0

3 years ago

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