All categories

3 years ago

a pro golfer hits 45.0-gram golf ball, giving its speed of 75.0 m/s. what is the momenntum has the golfer given to the ball

Chemistry

1 answer:

AfilCa [17]3 years ago

6 0

Momentum = mass x velocity. 45g = 0.045kg. 0.045 x 75 = 3.375 kgm/s

You might be interested in

Calcium and water form calcium hydroxide and hydrogen gas also called what type of reaction

Gekata [30.6K]

Reaction of calcium with water
Calcium reacts slowly with water. This is in contrast with magnesium, immediately above calcium in the periodic table, which is virtually unreactive with cold water. The reaction forms calcium hydroxide, Ca(OH)2 and hydrogen gas (H2).

4 0

3 years ago

¿En dónde se ubican los lípidos solubles?

tatyana61 [14]

Las vitaminas liposolubles (A, D, E, y K) son lípidos a base de isopreno que se almacenan en el hígado y la grasa.

7 0

3 years ago

What is the reaction of guanine and adenine

PtichkaEL [24]

Complementary Base Pairing. Specific pairs can only go together, so when guanine and adenine pair up, its Complementry Base Pairing :)

Hope this helps! Please correct me if im wrong :)

5 0

3 years ago

Read 2 more answers

Water has a specific heat of 4.186 J/g*C. How much energy would be required to raise the temperature of 10 g of water by 10 C?

Sladkaya [172]

Energy(heat) required to raise the temperature of water : 418.6 J

<h3>Further explanation </h3>

Heat can be calculated using the formula:

Q = mc∆T

Q = heat, J

m = mass, g

c = specific heat, joules / g ° C

∆T = temperature difference, ° C / K

Specific heat of water = 4.186 J/g*C.

∆T(raise the temperature) : 10° C

mass = 10 g

Heat required :

$\tt Q=m.c.\Delta T\\\\Q=10\times 4.186\times 10\\\\Q=418.6~J$

8 0

3 years ago

Part a use these data to calculate the heat of hydrogenation of buta-1,3-diene to butane. c4h6(g)+2h2(g)→c4h10(g)

Reptile [31]

<u>Answer:</u> The heat of hydrogenation of the reaction is coming out to be 234.2 kJ.

<u>Explanation:</u>

Enthalpy change is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as $\Delta H$

The equation used to calculate enthalpy change is of a reaction is:

$\Delta H_{rxn}=\sum [n\times \Delta H_{(product)}]-\sum [n\times \Delta H_{(reactant)}]$

For the given chemical reaction:

$C_4H_6(g)+2H_2(g)\rightarrow C_4H_{10}(g)$

The equation for the enthalpy change of the above reaction is:

$\Delta H_{rxn}=[(1\times \Delta H_{(C_4H_{10})})]-[(1\times \Delta H_{(C_4H_6)})+(2\times \Delta H_{(H_2)})]$

We are given:

$\Delta H_{(C_4H_{10})}=-2877.6kJ/mol\\\Delta H_{(C_4H_6)}=-2540.2kJ/mol\\\Delta H_{(H_2)}=-285.8kJ/mol$

Putting values in above equation, we get:

$\Delta H_{rxn}=[(1\times (-2877.6))]-[(1\times (-2540.2))+(2\times (-285.8))]\\\\\Delta H_{rxn}=234.2J$

Hence, the heat of hydrogenation of the reaction is coming out to be 234.2 kJ.

4 0

3 years ago