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Alika [10]
3 years ago
13

A car at rest ends accelerates for 12 seconds. After this time the car is going 36 m/s. What was its acceleration?

Chemistry
2 answers:
Zigmanuir [339]3 years ago
4 0

Acceleration is defined as velocity per unit time.

Acceleration=\frac{Velocity}{time}

a=\frac{dv}{dt}

Here, a=acceleartion,

v=velocity=36 m/s

t=time=12 s

a=\frac{dv}{dt}

a=\frac{36}{12}

a=3 ms⁻²

A car at rest ends accelerates for 12 seconds. After this time the car is going 36 m/s. So acceleration that is a=3 ms⁻².


liubo4ka [24]3 years ago
3 0

Using the equation of motion:

a = \frac{v-u}{t}

where a is acceleration, v is final velocity, u is initial velocity, and t is time

Given values are:

t = 12 sec, v= 36 m/s, u = 0 (because initially car was at rest)

Substituting the values in the formula:

a = \frac{36-0}{12} = 3 m/s^{2}

Hence, the acceleration of the car is 3 m/s^{2}.


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A lab group was supposed to make mL of a acid solution by mixing a solution, a solution, and a solution. However, the solution w
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Question: The question is not complete. Find below the complete question and the answer.

Alab group was supposed to make 14 mL of a 36% acid solution by mixing a 20% solution, a 26% solution, and a 42% solution. However, the 20% solution was mislabeled, and was actually a 10% solution, so the lab group ended up with 14 mL of a 34% acid solution, instead. If the augmented matrix that represents the system of equations is given below, what are the volumes of the solutions that should have been mixed? mL

Volume of 20% solution= ?

Volume of 26% solution = ?

Volume of 42% solution= ?   Round to the nearest whole number ml

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Volume of 20% solution= 3 mL

Volume of 26% solution = 1 mL

Volume of 42% solution= 10 mL

Explanation:

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3 years ago
) determine the theoretical yield and the percent yield if 21.8 g of k2co3 is produced from reacting 27.9 g ko2 with 29.0 l of c
Airida [17]
The Balanced Chemical Equation is as follow;

                         4 KO₂  +  2 CO₂    →    2 K₂CO₃  +  3 O₂

First find out the Limiting Reagent,
According to equation,

         284 g (4 moles) KO₂ reacted with  =  44.8 L (2 moles) of CO₂
So,
                  27.9 g of KO₂ will react with  =  X  L of CO₂


Solving for X,
                          X  =  (44.8 L × 27.9 g) ÷ 284 g

                          X  =  4.40 L of CO₂

Hence, to consume 27.9 g of KO₂ only 4.40 L CO₂ is required, while, we are provided with 29 L of CO₂, it means CO₂ is in excess and KO₂ is is limited amount, Therefore, KO₂ will control the yield of K₂CO₃. So,

According to eq.

         284 g (4 moles) KO₂ formed  =  138.2 g of K₂CO₃
So,
         27.9 g of KO₂ will form  =  X g of K₂CO₃

Solving for X,
                        X  =  (138.2 g × 27.9 g) ÷ 284 g

                        X  =  13.57 g of K₂CO₃

So, 13.57 g of K₂CO₃ formed is the theoretical yield.

%age Yield  =  13.57 / 21.8 × 100

%age Yield  =  62.24 %
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The hydrogen at 10 °C has slower-moving molecules than the sample at 350 K.

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Temperature in kelvin scale of the first sample = 10 + 273 = 283 K

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