Quantities must have different unit before they can be added or subtracted true or false

1 answer:

3 0

That statement is a false and untrue example of prevarication.

The truth is exactly the opposite. Quantities CAN NOT be added
or subtracted when their units are different. Before addition or
subtraction can be attempted, the quantities must have the SAME
units, and if that can't be arranged, then the quantities can't be
added or subtracted.

You might be interested in

The kinetic energy possessed by an object in motion is determined by which factor(s)?

jeka57 [31]

Answer:hiii

Explanation:

6 0

3 years ago

A standing wave on a string that is fixed at both ends has frequency 80.0 Hz. The distance between adjacent antinodes of the sta

Bingel [31]

Answer:

Speed of the wave in the string will be 3.2 m/sec

Explanation:

We have given frequency in the string fixed at both ends is 80 Hz

Distance between adjacent antipodes is 20 cm

We know that distance between two adjacent anti nodes is equal to half of the wavelength

So $\frac{\lambda }{2}=20cm$

$\lambda =40cm$

We have to find the speed of the wave in the string

Speed is equal to $v=\lambda f=0.04\times 80=3.2m/sec$

So speed of the wave in the string will be 3.2 m/sec

4 0

3 years ago

If you have 240.0 mL of water at 25.00 °C and add 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture? U

Rus_ich [418]

Answer: The final temperature of the mixture is 45.6°C

Explanation:

To calculate the mass of water, we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

Density of water = 1 g/mL

When volume is 240.0 mL

Putting values in above equation, we get:

$1g/mL=\frac{\text{Mass of water}}{240.0mL}\\\\\text{Mass of water}=(1g/mL\times 240.0mL)=240g$

When volume is 100.0 mL

Putting values in above equation, we get:

$1g/mL=\frac{\text{Mass of water}}{100.0mL}\\\\\text{Mass of water}=(1g/mL\times 100.0mL)=100g$

When two water solutions at different temperature are mixed, the amount of heat released by water present at higher temperature will be equal to the amount of heat absorbed by water present at lower temperature..

$Heat_{\text{absorbed}}=Heat_{\text{released}}$