-23
You don't. You solve it. u - v^2 - u + v^2 = 0
You solve the equation for kinetic energy for mass. KE = (1/2) m v2 (1/2) m v2 = KE m = 2 KE / v2
2 16/25 = 2.64
There is nothing to solve! 2.12 = 212/100 = 53/25
25% = 0.2560.5 x 0.25 = 15.125
To solve Boyle's Law equation for V2, first write the equation as P1V1 = P2V2. Then rearrange it to isolate V2 on one side, dividing both sides by P2 to solve for V2, which will be V2 = (P1 * V1) / P2.
You don't. You solve it. u - v^2 - u + v^2 = 0
100 V2 - 25 W2 = (10V + 5W) (10V - 5W)Another way to show it:100 V2 - 25 W2 = 25 (4 V2 - W2) = 25 (2V - W) (2V + W)
You solve the equation for kinetic energy for mass. KE = (1/2) m v2 (1/2) m v2 = KE m = 2 KE / v2
For all dilution/ concentration problems you use the simple equation: M1V1 = M2V2 2.40*V2 = 8.25*25 V2 = (8.25*25)/2.40 V2 = 85.9mL Final volume will be 86mL.
type in 25/pi
the V2 rocket was bigger and faster than the V1 flying bomb. the V1 being a flying bomb was smaller and had a pulse jet engine and the V2 which was a rocket had a bigger rocket engine. ACTUAL SIZE COMPARISON: V1: Length: 25' 4" wingspan: 8.32 meters V2: length 14 m (45 ft 11 in)
Use Charles's Law: V1 / T1 = V2 / T2 Constant pressure must be kept. Absolute temp. must be used. T1 = 0 + 273 = 273 degr.K T2 = 200 + 273 = 473 degr.K 25 L / 273 K = V2 / 473 K V2 = 25 x 473 / 273 = 43.315 L (final volume).
The volume of the gas will decrease proportionally to the increase in pressure, following Boyle's Law. Using the formula P1V1 = P2V2, where P1 = 12 ATM, V1 = 23 L, and P2 = 14 ATM, we can solve for V2 to find the new volume of the gas. Solving for V2 gives V2 = (P1)(V1) / P2 = (12)(23) / 14 = 19.71 liters.
2 16/25 = 2.64
Using the ideal gas law (PV = nRT) and since the temperature is constant, the initial and final conditions of the gas can be related through (P1V1) = (P2V2). Given: P1 = 0.93 atm V1 = 9.00 m^3 P2 = 1 atm (standard pressure) V2 = unknown Rearranging the equation to solve for V2 gives: V2 = (P1V1) / P2 Substitute the values and solve: V2 = (0.93 atm * 9.00 m^3) / 1 atm V2 = 8.37 m^3 Therefore, the volume of the gas at standard pressure is 8.37 m^3.
To prepare a 10 ppm dilution from a 100 ppm stock solution, you can use the dilution equation: C1V1 = C2V2, where C1 is the concentration of the stock solution, V1 is the volume of the stock needed, C2 is the desired concentration, and V2 is the final volume. Here, C1 is 100 ppm, C2 is 10 ppm, and V2 is 25 ml. Rearranging the equation to solve for V1 gives you V1 = (C2 * V2) / C1 = (10 ppm * 25 ml) / 100 ppm = 2.5 ml. Therefore, you need to take 2.5 ml of the 100 ppm solution and dilute it with 22.5 ml of solvent (water or another appropriate diluent) to achieve a total volume of 25 ml at 10 ppm.